DHºformation = 0 for both Zn and Cu because these are in the most stable state.

Calculate the standard heat of reaction for the following reaction:

Zn(s) + Cu2+(aq) &#8594; Zn2+(aq) + Cu(s)

5) The standard enthalpy of formation of propene, C3H6, is +20.6 kJ/mole. Calculate the heat of combustion of one mole of C3H6. The heats of formation of CO2(g) and H2O(l) are -394 kJ/mole and -285.8 kJ/mole respectively.-7.53 kJ/mole?

6) The standard enthalpy of formation of propane, C3H8, is -103.6 kJ/mole. Calculate the heat of combustion of one mole of C3H8. The heats of formation of CO2(g) and H2O(l) are -394 kJ/mole and -285.8 kJ/mole respectively.

7) Using the following information calculate the heat of formation of NF3.

NH3(g) + 3 F2(g) &#8594; NF3(g) + 2 HF(g)

DHº = -604.8 kJ

DHºf NH3(g) = -46.19 kJ/mole

DHºf HF(g) = -269 kJ/mole

8) Using the following information calculate the heat of formation of Fe2O3.

Fe2O3(s) + 3 CO(g) &#8594; 2 Fe(s) + 3 CO2(g)

DHº = -24.8 kJ

DHºf CO(g) = -110.5 kJ/mole

DHºf CO2(g) = -393.5 kJ/mole

9) Using the given standard enthalpies of formation and the heat of reaction, calculate the heat of formation of HNO3(aq).

3 NO2(g) + H2O(l) &#8594; 2 HNO3(aq) + NO(g)

DHº = -138.5 kJ

DHºf NO2(g) = +33.84 kJ/mole

DHºf NO(g) = +90.37 kJ/mole

DHºf H2O(l) = -285.85 kJ/mole

10) Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

Fe2O3(s) + 2 H2(g) &#8594; 3 Fe(s) + 3 H2O(l)

DHºf Fe2O3(s) = -822.2 kJ/mole

DHºf H2O(l) = -285.9 kJ/mole

11) Calculate Hof (kJ) for the following reaction from the listed standard enthalpies of formation:

CO(g) + NH3(g) &#8594; HCN(g) + H2O(g)

DHºf CO(g) = -110.5 kJ

DHºf NH3(g) = -46.1 kJ

DHºf HCN(g) = +135.1 kJ

DHºf H2O(g) = -241.8 kJ

12) Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

C3H6O(l) + 4 O2(g) &#8594; 3 CO2(g) + 3 H2O(l)

DHºf CO2(g) = -393.5 kJ/mole

DHºf H2O(l) = -285.8 kJ/mole

DHºf C3H6O(l) = -249.5 kJ/mole

13) Calculate the heat of reaction (kJ) using the listed heats of formation:

CH4(g) + 4 F2(g) &#8594; CF4(g) + 4 HF(g)

DHºf CH4 = -74.81 kJ/mole

DHºf CF4 = -925.0 kJ/mole

DHºf HF = -271.1 kJ/mole

14) Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

2 C3H6(g) + 9 O2(g) &#8594; 6 CO2(g) + 6 H2O(l)

DHºf C3H6(g) = +53.5 kJ/mole

DHºf CO3(g) = -393.5 kJ/mole

DHºf H2O(l) = -285.9 kJ/mole

15) Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction: